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Ammonia Production

Rate Limitations in Ammonia Production Redefined by Catalyst

| Editor: Constanze Schmitz

Hideo Hosono and colleagues at Tokyo Institute of Technology and the Japan Science and Technology Agency in Japan, University College London in UK and Pacific Northwest National Laboratory in US investigated Ru/C12A7:e- as a catalyst in ammonia production.
Hideo Hosono and colleagues at Tokyo Institute of Technology and the Japan Science and Technology Agency in Japan, University College London in UK and Pacific Northwest National Laboratory in US investigated Ru/C12A7:e- as a catalyst in ammonia production. (Source: Tokyo Institute of Technology)

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Researchers at theTokyo Institute of Technology developed a catalyst promoting the dissociation of the nitrogen bond in ammonia production so that it is no longer the step limiting the rate of the reaction.

Tokyo/Japan — A collaboration of researchers in Japan, the UK and the US have developed a catalyst that is so effective towards the break of the nitrogen triple bond so that this is no longer the rate-limiting step of the reaction. Ammonia (NH3) is crucial for the industrial synthesis of fertilizers and pharmaceuticals so that ways to improve its production from molecular nitrogen and hydrogen are in high demand. So far the main challenge has been breaking the triple bond in nitrogen molecules, which is the strongest bond in a molecule of two atoms.

Certain oxides can be very effective at enhancing the catalytic activity of ruthenium and iron but they are unstable in ammonia synthesis conditions. Recently the electride 12CaO·7Al2O3:e- (C12A7:e-) - an ionic compound with an electron acting as the negative ion – was found to be stable at room temperature. The discovery prompted Hideo Hosono and colleagues at Tokyo Institute of Technology and the Japan Science and Technology Agency in Japan, University College London in UK and Pacific Northwest National Laboratory in US to investigate Ru/C12A7:e- as a catalyst in ammonia production.

The researchers examined the N2 isotope exchange and hydrogen adsorption/desorption reactions. They observed a remarkable level of catalytic activity at less than half the activation energy of other catalysts. In addition the catalyst did not degrade due to hydrogen poisoning as is usually the case for ruthenium-based catalysts.

Further studies and density functional calculations suggested a mechanism for the reaction. “Fast N2 cleavage is ensured by highly efficient electron transfer from C12A7:e- to N2 molecules adsorbed on the Ru nanoparticles,” the researchers conclude in their report. “As a result, the bottleneck in the NH3 synthesis reaction is shifted from the N-N triple bond dissociation to the formation of nitrogen-hydrogen species.”

Haber-Bosch production process

Both iron and ruthenium are well known catalysts for the break of the nitrogen bond. However ruthenium-based catalysts are highly prone to hydrogen poisoning where hydrogen adsorbs to the catalyst, so that for over a century iron-based catalysts have remained central to the widely implemented ammonia production process developed by Fritz Haber and Carl Bosch in 1909.

Alkali and alkaline earth metal oxides enhance ruthenium and iron catalysts by donating electrons into the ‘antibonding orbitals’ of the nitrogen, weakening the bond. This is referred to as the electronic promoting effect but has so far been difficult to harness for ammonia synthesis because the oxides are unstable in the reaction conditions.

Catalyst structure

The promoter the researchers investigated is a combination of oxides of calcium (an alkaline earth metal) and aluminium in the form of an electride - 12CaO·7Al2O3:e- (C12A7:e-). The same ionic compound can be used with oxides or hydrides acting as the anion instead of an electron as in the electride studied, but these are far less effective.

The crystal structure of C12A7:e- consists of a positively charged framework having the chemical formula [Ca24Al28O64]4+, and four extra framework electrons accommodated in the cages as counter ions. This structure has uniquely versatile characteristics for the exchange of negatively charged ions.

Shifting the bottleneck

The researchers monitored N2 isotope exchange and hydrogen adsorption/desorption reactions. From these observations the researchers determined that breaking the nitrogen triple bond was no longer the rate-limiting step of ammonia synthesis with the Ru/C12A7:e-. Instead they suggest that the subsequent formation of the nitrogen-hydrogen bond in ammonia is now the bottleneck in the process.

The researchers also calculated the order of the reaction from the effect on the rate as the concentrations of the chemicals were varied. The catalyst had a lower reaction order for nitrogen than other catalysts suggesting a different mechanism, and that the nitrogen populates the catalyst more densely than for other catalysts.

Catalyst stability

The Ru/C12A7:e- catalyst was not subject to hydrogen poisoning and remained active at high pressure. The researchers suggest that the fast formation of ammonia on the ruthenium surface limits hydrogen being incorporated into the catalyst so that its activity remains unchanged.

Further studies suggest that the reversible hydrogen storage-release properties are responsible for the reaction mechanism of the new catalyst. This mechanism switches at temperatures below 593 K at which temperatures the catalyst becomes prone to hydrogen poisoning like other catalysts.

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